Reactions of Methanesulfonic Acid with Amines ... - ACS Publications

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Reactions of Methanesulfonic Acid with Amines and Ammonia as a Source of New Particles in Air Haihan Chen, Mychel E. Varner, R. Benny Gerber,* and Barbara J. Finlayson-Pitts* Department of Chemistry, University of California, Irvine, California 92697, United States S Supporting Information *

ABSTRACT: New particle formation (NPF) from gaseous precursors as a significant source of aerosol needs to be better understood to accurately predict the impacts on visibility, climate change, and human health. While ternary nucleation of sulfuric acid, amines/NH3, and water is recognized as a significant driver for NPF, increasing evidence suggests a contribution from methanesulfonic acid (MSA) and amines under certain conditions. Here we report the formation of particles 2.5−10 nm in diameter from the reactions of MSA with methylamine (MA), dimethylamine (DMA), and NH3 at reaction times of 2.3−7.8 s in a flow reactor and compare these particles with those previously reported to be formed from reaction with trimethylamine (TMA). The effects of water vapor and concentrations of gaseous precursors on the particle number concentration and particle size were studied. The presence of water significantly enhances particle formation and growth. Under similar experimental conditions, particle number concentrations decrease in the order MA ≫ TMA ≈ DMA ≫ NH3, where NH3 is 2−3 orders of magnitude less efficient than DMA. Quantum chemical calculations of likely intermediate clusters were carried out to provide insights into the role of water and the different capacities of amines/NH3 in particle formation. Both gas-phase basicity and hydrogen-bonding capacity of amines/NH3 contribute to the potential for particles to form and grow. Our results indicate that, although amines typically have concentrations 1−3 orders of magnitude lower than that of NH3 in the atmosphere, they still play an important role in driving NPF.

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sufficient to explain particle formation in the atmosphere.25 Amines can play a more important role in NPF,24,26−32 possibly due to the stronger bonds they form with H2SO4 compared to NH3.27 Laboratory experiments have demonstrated that amines are more effective in forming particles with H2SO4.24,26,28−30,32 Field studies have shown that aminium salts are widely present in ambient particles,31,33−35 and NPF is correlated with the presence of amines.36,37 In addition, amines have been found to effectively displace NH3 in ammonium bisulfate clusters/ particles,38−41 with a close-to-collision-limited rate for small clusters.38,39 Thus, aminium salts are likely to be present even if ammonium salts are initially formed. Ammonia and amines are emitted from a wide range of sources, including biological processes in the ocean, animal husbandry, industrial operations, fuel and biomass burning, and agricultural activities.42 The concentration of gas-phase amines in the atmosphere is typically at least one order of magnitude smaller than that of NH3, but this may increase with their use in CO2 capture and storage as the technology becomes more widely adopted.42−45

INTRODUCTION Atmospheric particles have well-known deleterious effects on human health1,2 and visibility.3−5 Those particles can globally affect radiative forcing and climate by absorbing and scattering solar radiation as well as by acting as cloud condensation nuclei (CCN) to change cloud coverage and properties.6−8 However, great uncertainties remain in the mechanisms of formation of atmospheric particles, and these preclude accurate assessment of the impacts of atmospheric particles on human health, visibility, and climate.9 New particle formation (NPF) from gasto-particle conversion represents a significant source of atmospheric particles10,11 and contributes up to half of global CCN.8,12 Understanding the potential species driving NPF and the underlying mechanisms is therefore critical for prediction and control of climate change.9,10 Sulfuric acid (H2SO4) formed from SO2 oxidation in air has been well recognized as a key species driving NPF.13−15 The reaction of H2SO4 with ammonia (NH3) and amines represents the initial step in gas-to-particle conversion to form small clusters,10,11 which can further grow into detectable size particles in the atmosphere. Low-volatility, high-molecularweight organic compounds are likely also involved.16−20 Although ternary nucleation of H2SO4−NH3−H2O has been shown to enhance particle formation by orders of magnitude compared to binary nucleation of H2SO4−H2O,21−26 it is not © 2015 American Chemical Society

Special Issue: Bruce C. Garrett Festschrift Received: July 31, 2015 Revised: September 17, 2015 Published: September 17, 2015 1526

DOI: 10.1021/acs.jpcb.5b07433 J. Phys. Chem. B 2016, 120, 1526−1536

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The Journal of Physical Chemistry B

ring inlets (ring A and ring B) to make the total flow in the flow reactor 17 slpm. Thus, MSA was mixed with water vapor before reacting with the specific amines/NH3 for experiments under humid conditions. All experiments were performed at ambient temperature. Because of wall losses of MSA, the gas flow of MSA was first introduced into the flow reactor to passivate the walls for 2−3 days. The gas flow of the selected amines/NH3 was then introduced to initiate particle formation. Particle formation and growth as a function of time were monitored by adjusting the distance between the sampling tube and the spokes inlet D. A previously determined conversion factor (0.14 s cm−1) was used to convert the distance to reaction times.51 All of the flows were controlled by high-precision mass flow controllers (Alicat or MKS), and were checked with a flow meter (Gilibrator 2; Sensidyne) prior to each experiment. Dry air was further purified through a purge gas generator (model 75-62; Parker Balston), carbon/alumina media (Perma Pure, LLC), and a 0.1 μm filter (DIF-N70; Headline Filters). Humid air was achieved by passing a portion of the dry air through a water bubbler filled with Nanopure water. The relative humidity (RH) was monitored with a RH probe (model HMT338; Vaisala) at the downstream end of the reactor. The gas-phase MSA flow was generated by passing dry purified air over liquid MSA (99.0%, Fluka) contained in a trap. The gasphase amines or ammonia were added into the system from gas tanks (1−10 ppm in N2, Airgas) without further purification. To determine the concentration of gas-phase MSA, the gas flow out of the MSA trap was first passed through a 0.45 μm Durapore filter (Millex-HV) for 5−15 min for collection. The collected MSA was extracted with 10 mL of Nanopure water, and then the extract was analyzed using ultra-performance liquid chromatography coupled with tandem mass spectrometry (UPLC-MS/MS, Waters). The concentrations of MA, DMA, and NH3 were determined as previously described.65 Briefly, the amines/NH3 from the source were collected for 20−120 min using a high-concentration cartridge that contains a weak cation exchange resin, extracted with 10 mL of 0.1 M oxalic acid (Fluka), and analyzed with ion chromatography (Metrohm). The measured concentrations of ammonia and the amines were typically lower than values provided by the manufacturers. The analysis also confirmed that no significant contaminant of other amines or NH3 was present in the selected amine/NH3 (18.0 MΩ cm; Model 7146; Thermo Scientific) and dried with purified air with the water jacket kept at ∼70 °C. In all experiments, the mixture of purified air and MSA flow was introduced from the spokes C at a total flow of 2 slpm (standard liter per minute at 25 °C and 101.32 kPa), and the mixture of purified air and the selected amines/NH3 from the spokes D at a total flow of 1 slpm. Dry/humidified air at a total flow of 14 slpm was introduced from the upstream 1527


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The Journal of Physical Chemistry B be ∼2.5 nm. All particle diameters reported here are geometric mean mobility diameters obtained from the SMPS.

vapor. Clearly, particle formation and growth are much more favorable when water is present. An enhancement effect of water vapor on particle formation has also been reported in previous H2SO4-amines studies.24,28,29,70,71 In some cases in this study, there are spikes in the size distributions of particles below the SMPS cutoff of 2.5 nm at short reaction times (Figure 1). This suggests the presence of smaller particles or clusters 2.5 nm for different amines/NH3 is shown in Figure 6. Results from two separate experiments for each base are in good agreement. The different basic species show different abilities in forming particles with MSA. Consistent with previous studies in the H2SO4−amines/NH3 system,24,26−30 amines are much more effective than NH3 in promoting particle formation from MSA. Of the three amines studied here, MA is by far the most effective, followed by TMA and DMA. Theoretical Calculations. Both gas-phase basicity and hydrogen-bonding capacity can contribute to the potential for particles to form and grow. With increasing gas-phase basicity, the reaction with MSA is more exothermic. With increasing hydrogen-bonding capacity, the sites for addition of molecules from the gas phase increase in number. However, neither gasphase basicity, which increases with the number of methyl groups for the series MA < DMA < TMA, nor hydrogenbonding capacity, which decreases with the number of methyl

Figure 4. Particle formation rates as a function of H2O observed in the MSA−base−H2O system. Error bars represent two standard deviations and lie within the symbols in some cases. The basic species are MA, DMA, TMA, and NH3. Experiments were repeated at least twice under varied concentrations of MSA, base, and H2O for each type of basic species. The power dependency (n ± 2σ) and the concentrations of MSA and the base for each experiment are shown. The TMA data are from ref 50.

Figure 5. (a) Number concentrations and (b) diameters of particles measured by SMPS from the reaction of 1.0 ppb MSA with variable concentrations of MA as a function of reaction time at 55% RH. The lines between data points are drawn to as guides to the eye. Uncertainties represent two standard deviations from triplicate SMPS measurements and lie within the symbols in some cases. Measurements of the diameters have high uncertainties at short reaction times due to the experimental challenges of detecting low particle numbers, and those data have been disregarded in drawing lines. 1530


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= −29 kcal mol−1, ΔG = −16 kcal mol−1). MSA addition to the TMA ion pair (MeSO3−)·(Me3NH+) occurs through hydrogen bonding of the acidic −OH group to an −SO group of the anion (Figure 7a). This leads to a somewhat weaker interaction compared to the MA and DMA cases where an additional hydrogen bond to an available −NH group is formed (Figures 8a and 9a), but MSA is still strongly bound to the TMA ion pair (ΔH = −25 kcal mol−1, ΔG = −12 kcal mol−1). As MSA addition is favorable in all cases, and not less favorable for DMA where there is limited particle formation under dry conditions, we move to the next step: amine addition to the (MSA)2· (amine) cluster. Structures for (MSA)2·(TMA)2 isomers are also included in Figure 7. Addition of a second TMA molecule may form an initial intermediate (Figure 7b) which is energetically stable, ΔH = −5 kcal mol−1 (ΔG = +4 kcal mol−1). This intermediate (Figure 7b) may then isomerize to the significantly more stable (MeSO3−)2·(Me3NH+)2 cluster (Figure 7c), ΔH = −21 kcal mol−1 (ΔG = −9 kcal mol−1) relative to (MSA)2·(TMA) + TMA. The addition of MA to a (MSA)2·(MA) cluster to form a stable (MeSO3−)2·(MeNH3+)2 (Figure 8c) may proceed through a weakly bound complex (Figure 8b) similar to that of TMA (Figure 7b). The binding enthalpy of this complex is similar to the TMA case, ΔH = −5 kcal mol−1 (ΔG = +5 kcal mol−1). However, in the case of MA an alternate route for cluster growth may facilitate particle formation under dry conditions. The (MSA)2·(MA) cluster consists of a (MeSO3−)· (MeNH3+) ion pair similar to the TMA cluster, but with the additional −NH groups of MA, the MSA molecule is hydrogenbonded to both the anion and cation (Figure 8a). The MeNH3+

Figure 6. Comparison of particle formation rates (J>2.5 nm) for MSA with the basic species, i.e., MA, DMA, TMA, and NH3, at ∼55% RH. The initial concentration of MSA is 1.7 ppb. Two separate experiments were performed for each base, and the data are represented as symbols with different shapes.

groups for the series MA > DMA > TMA, alone can explain the observed lack of particle formation for DMA relative to both TMA and MA under dry conditions. Calculations for alternating addition of acid and base molecules to the initial acid−base ion pair were carried out in an attempt to identify differences in the growth mechanisms that would explain the differences in particle formation rates observed experimentally for the series of amines. The stability of the cluster formed from addition of MSA to the initial acid−amine ion pair is similar for MA and DMA (MA: ΔH = −29 kcal mol−1, ΔG = −15 kcal mol−1; DMA: ΔH

Figure 7. Structures for (MSA)2·(TMA) and isomers of (MSA)2·(TMA)2: (a) (MSA)2·(TMA), (b) the initial complex for addition of TMA at the hydrogen-bonded MSA of (MSA)2·(TMA), and (c) the double ion pair cluster of (MSA)2·(TMA)2. Red represents MSA, green the amine. 1531


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Figure 8. Structures for (MSA)2·(MA) and isomers of (MSA)2·(MA)2: (a) (MSA)2·(MA), (b) the initial complex for addition of MA at the hydrogen-bonded MSA of (MSA)2·(MA), (c) the double ion pair cluster of (MSA)2·(MA)2, and (d) the initial complex for addition of MA at the −NH group of the cation of (MSA)2·(MA). Red represents MSA, green the amine.

(MSA)2·(MA)2 and (MSA)2·(DMA)2 clusters (ΔH = −36 and −37 kcal mol−1, respectively) are close and are significantly larger than the binding energy informing (MSA)2·(TMA)2 due to a cyclic hydrogen-bonding structure between alternating cations and anions.72 However, the availability of an NH group that is not hydrogen-bonded in the MA cluster may lead to an extended hydrogen-bonding network, an arrangement seen in the crystal structure of ammonium methanesulfonate.75 While growth of a perfect crystal may not occur in this case, the additional hydrogen-bonding site may play a role in more effectively growing the MSA-MA clusters to detectable sizes even under dry conditions. For DMA, the large binding energy between MSA-DMA ion pairs enhances the formation and stability of (MSA)2·(DMA)2 clusters, so that these double ion pairs may play an important role in growth to detectable particle sizes. Coagulation of two of these larger clusters may exhibit steric effects, whereas growth through single ion pairs for TMA would be less sterically hindered, leading to more rapid formation of detectable particles in the TMA system. Structures of (MSA)2·(DMA)·(H2O)2 and (MSA)2·(DMA)2· (H2O)2 illustrating how water facilitates amine addition are included in Figure 10. The incorporation of water into the (MSA)2·(DMA) cluster provides hydrogen-bonding sites for initial addition from the gas phase. Addition of DMA to (MSA)2·(DMA)·(H2O)2 (Figure 10a) leads directly to a very stable cluster (Figure 10b: ΔH = −27 kcal mol−1, ΔG = −16 kcal mol−1). A weakly bound intermediate, analogous to that of the dry cluster, was not identified in the case of the hydrated clusters.

cation has a remaining hydrogen-bonding site available for addition of the second MA molecule from the gas phase. Addition of the second amine at the cation (Figure 8d) forms a more stable intermediate (ΔH = −11 kcal mol−1 and ΔG = −2 kcal mol−1) than at the hydrogen-bonded MSA (Figure 8b: ΔH = −5 kcal mol−1, ΔG = +5 kcal mol−1). Binding of DMA to a (MSA)2·(DMA) cluster (Figure 9a) to form (MSA)2·(DMA)2 (Figure 9c) either at the hydrogenbonded MSA (Figure 9b: ΔH = −8 kcal mol−1, ΔG = +2 kcal mol−1) or at the cation (Figure 9d: ΔH = −13 kcal mol−1, ΔG = −2 kcal mol−1), is slightly greater than the corresponding MA system. The two routes for cluster growth, addition either at the cation or at the neutral acid molecule, both seem to be feasible for the MSA−DMA system, and potentially more likely based on enthalpies of formation of the complexes. The conclusion from these calculations is that understanding the anomalous dry behavior of DMA will require consideration of intermediates at the level of four or more molecule clusters. Dawson et al.72 described structures and binding for (MSA)2· (MA)2, (MSA)2·(DMA)2, and (MSA)2·(TMA)2 clusters, including speculation on the nature of interactions in extended systems. The endothermicity for dissociation of (MSA)2· (TMA)2 to (MeSO3−)(Me3NH+) ion pairs, ΔH = 24 kcal mol−1, is similar to the exothermicity of TMA addition to (MSA)2·(TMA) presented above. Due to the lack of hydrogen bonds between (MeSO3−)(Me3NH+) ion pairs, the single ion pair formed on fragmentation may then play a significant role in growing the stabilized clusters to detectable size particles.50 For comparison, the binding energies of ion pairs in forming 1532


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Figure 9. Structures for (MSA)2·(DMA) and isomers of (MSA)2·(DMA)2: (a) (MSA)2·(DMA), (b) the initial complex for addition of DMA to the hydrogen-bonded MSA of (MSA)2·(DMA), (c) the double ion pair cluster of (MSA)2·(DMA)2, and (d) the initial complex for addition of DMA at the −NH group of the cation of (MSA)2·(DMA). Red represents MSA, green the amine.

Figure 10. Structures for (a) (MSA)2·(DMA)·(H2O)2 and (b) (MSA)2·(DMA)2·(H2O)2. Red represents MSA, green the amine, blue the H2O.

The binding of water to the initial ion pair is slightly greater for MA and DMA (ΔH = −15 kcal mol−1, ΔG ≈ −5 kcal mol−1) than for TMA (ΔH = −11 kcal mol−1, ΔG ≈ −2 kcal mol−1). While there is not a significant difference in the binding energy of water to the MA vs DMA ion pair, the MA ion pair has an additional hydrogen-bonding site that may increase the chances of picking up water from the gas phase. If hydrated clusters are formed more quickly or are more stable, and hydration aids cluster growth, this could explain the faster formation of detectable particles from MA (Figure 2a) compared to DMA (Figure 2b) and TMA (Figure S2). The

growth of DMA and TMA particles is also significantly faster than the MA particles (Figure 2 and S2). This can be due to (1) a larger contribution of growth from water because of their higher hygroscopicities,72 (2) a larger molecular volume, and/ or (3) smaller particle formation rates so that higher concentrations of gas precursors and small clusters that can contribute to growth are left in the DMA and TMA systems. It is noteworthy that at essentially the same concentration of MSA (Table 1), NH 3 needs to be at much higher concentrations (18 ppb) than MA, DMA or TMA (2.5 ppb) to form comparable number concentrations of particles (Figure 1533


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concentrations in the atmosphere, are expected to play a significant role in the initial stages of NPF.

2c). Clearly, NH3 is much less effective in particle formation similar to the case of H2SO4-amines/NH3 studies.24,26−30,32 The formation energies of MSA·NH3 and MSA·NH3·H2O were calculated to be ΔH = −14 kcal mol−1 (ΔG = −5 kcal mol−1) and ΔH = −26 kcal mol−1 (ΔG = −6 kcal mol−1), respectively, significantly lower than the corresponding clusters of amines (Table 2). The formation of initial clusters is less favorable in the NH3 system, resulting in less effectiveness in NPF (Figure 6).

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S Supporting Information *

The Supporting Information is available free of charge on the ACS Publications website at DOI: 10.1021/acs.jpcb.5b07433. Figure S1, schematic of the flow reactor; Figure S2, particle formation and growth in the MSA−TMA system; detailed description of the theoretical methods; and Cartesian coordinates and B3LYP-D3/6-31++G** and RIMP2/aug-cc-pV(T+d)Z electronic energies of the structures in Figures 7−10 (PDF)

Table 2. Formation Energies and Enthalpies for Initial Clusters of MSA with Amines/Ammonia MSA·base

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MSA·base·H2O

base

ΔH (kcal mol−1)

ΔG (kcal mol−1)

ΔH (kcal mol−1)

ΔG (kcal mol−1)

MA DMA TMA NH3

−18 −21 −22 −14

−7 −9 −12 −5

−32 −36 −34 −26

−11 −15 −14 −6

ASSOCIATED CONTENT

AUTHOR INFORMATION

Corresponding Authors

*For theory, R.B.G.: E-mail [email protected]. *For experiments, B.J.F.-P.: E-mail bjfi[email protected], phone (949) 824-7670, fax (949) 824-2420. Notes

The authors declare no competing financial interest.

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If gas-phase basicity and hydrogen-bonding capacity are the two competing factors in particle formation and growth for the series of amines studied here, the success of MA in forming particles indicates that the hydrogen-bonding capacity of the amine plays a larger role, though the ineffectiveness of ammonia indicates that threshold basicity is required. This differs from the case of sulfuric acid,29,32 which provides greater hydrogen-bonding capacity, so it is not surprising that the relative effects of amines are different than for MSA. The conceptual approach taken in this paper involves calculations for small clusters, with extrapolation to likely growth possibilities. Calculations for larger particles are obviously very desirable. One appealing direction is to carry out calculations for crystalline particles, using periodic boundary conditions. As the crystalline salt is likely not the most relevant model for growth of the early-stage clusters and at the disordered surface, and high-level calculations with periodic boundary conditions remain a challenge for systems of this size, this approach was not pursued here, but it is a very interesting direction for the future.

ACKNOWLEDGMENTS The authors are grateful to the National Science Foundation (grant nos. 0909227 and 1443140) for funding. We thank Metrohm USA for their support and help in ion chromatography analysis. Computational resources include the Greenplanet cluster at University of California, Irvine, the CSC cluster Taito in Helsinki, Finland, and those of the Fritz-Haber Center in Jerusalem, Israel. It is a pleasure to dedicate this paper to Bruce Garrett, whose contributions from molecular interactions with liquid surfaces to nucleation theory and particle growth greatly impacted the study of atmospheric chemistry and have been a major influence on work done at AirUCI. His support of a strong interaction between theory and experiment is one important example.

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ATMOSPHERIC IMPLICATIONS Particle formation and growth are observed for reactions of MSA with ammonia and three small alkyl amines, MA, DMA, and, as reported earlier,50 TMA. Thus, the reaction of MSA with ammonia and amines must contribute to NPF in the atmosphere. Consistent with the previous studies,50,52 water shows a significant enhancement effect on particle formation and growth from MSA. Relative humidity is therefore expected to be a critical factor affecting NPF in the atmosphere. Similar to previous studies on the H2SO4−amines/NH3 system,24,26−30 amines are much more effective in forming particles with MSA than ammonia. Different bases show capacities in NPF with MSA in the order of MA ≫ TMA ≈ DMA ≫ NH3. While particle formation rates of amines with MSA are about 2−3 orders of magnitude higher than that of ammonia, field measurements in agricultural, ocean, and landfill areas usually show concentrations of amines approximately 1−3 orders of magnitude lower than those of ammonia.42 Together these indicate that amines, despite having relatively smaller 1534


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